Download chem 102

Chemistry 100(02) Fall 2014
Instructor: Dr. Upali Siriwardane
e-mail: [email protected]
Office: CTH 311
Phone 257-4941
Office Hours: M,W, 8:00-9:30 & 11:30-12:30 a.m
Tu,Th,F 8:00 - 10:00 a.m. Or by appointment
Test Dates:
September 29, 2014 (Test 1): Chapter 1 & 2
October 20,
2014 (Test 2): Chapter 3 & 4
November 12, 2014 (Test 3) Chapter 5 & 6
November 13, 2014 (Make-up test) comprehensive:
Chapters 1-6 9:30-10:45:15 AM, CTH 328
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Text Book & Resources
REQUIRED :
Textbook: Principles of Chemistry: A Molecular Approach,
2nd Edition-Nivaldo J. Tro - Pearson Prentice Hall and also
purchase the Mastering Chemistry
Group Homework, Slides and Exam review guides and
sample exam questions are available online:
http://moodle.latech.edu/ and follow the course information
links.
OPTIONAL :
Study Guide: Chemistry: A Molecular Approach, 2nd EditionNivaldo J. Tro 2nd Edition
Student Solutions Manual: Chemistry: A Molecular
Approach, 2nd Edition-Nivaldo J. Tro 2nd
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Chapter 3. Molecules, Compounds, and Chemical
Equations
3.1 Hydrogen, Oxygen, and Water…………………………….
3.2 Chemical Bonds……………………………………………
3.3 Representing Compounds: Chemical Formulas and Molecular Models..
3.4 An Atomic-Level View of Elements and Compounds……………..
3.5 Ionic Compounds: Formulas and Names……………………
3.6 Molecular Compounds: Formulas and Names………………………
3.7 Formula Mass and the Mole Concept for Compounds…………
3.8 Composition of Compounds……………………………..
3.9 Determining a Chemical Formula from Experimental Data………
3.10 Writing and Balancing Chemical Equations……………………
3.11 Organic Compounds……………………….
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Chapter 3. KEY CONCEPTS
• Writing Molecular and Empirical
Formulas (3.3)
• Classifying Substances as Atomic
Elements, Molecular Elements,
Molecular Compounds, or Ionic
Compounds (3.4)
• Writing Formulas for Ionic
Compounds (3.5)
• Naming Simple Ionic Compounds
(3.5)
• Naming Ionic Compounds Containing
Polyatomic Ions (3.5)
• Naming Molecular Compounds (3.6)
• Naming Molecular Compounds (3.6)
• Naming Acids (3.6)
• Calculating Formula Mass (3.7)
• Using Formula Mass to Count
Molecules by Weighing (3.7)
• Calculating Mass Percent
Composition (3.8)
CHEM 100, Fall 2014 LA TECH
• Using Mass Percent Composition
as a Conversion Factor (3.8)
• Using Chemical Formulas as
Conversion Factors (3.8)
• Obtaining an Empirical Formula
from Experimental Data (3.9)
• Calculating a Molecular Formula
from an Empirical Formula and
Molar Mass (3.9)
• Obtaining an Empirical Formula
from Combustion Analysis (3.9)
• Balancing Chemical Equations
(3.10)
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CHEMICAL BONDS:
THE FORCE BETWEEN ATOMS
What Makes a Molecule?
Structural formula
Space-filling model
Methane, CH4
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Molecular Compounds:
Nonmetal + Nonmetal
Name the most “metallic” of the nonmetals first.
Change the ending of the nonmetal to “IDE.”
Indicate the number of atoms of the nonmetal by Latin prefixes.
 Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
 Examples:
– P 2 O 5 : diphosphorous pentaoxide
– CO: carbon monoxide
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Naming Binary
Molecular-Covalent Compounds
For compounds composed of two non-metallic
elements the more metallic element is listed
To designate the multiplicity of an element
Greek prefixes are used:
mono  1; di  2; tri  3; tetra  4;
penta  5; hexa  6; hepta  7; octa 
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1) H2O, Na3PO4, HCl, C2H6, NH3, KCl, CH4, NH4Cl, C6H12O6, BrassCuxZny, SO3, NaCl, CO2
Identify the types of compounds in the above list:
Molecular compound:
Ionic compound:
Alloy:
Organic:
Inorganic:
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H2O, Na3PO4, HCl, C2H6, NH3, KCl, CH4, NH4Cl, C6H12O6, BrassCuxZny, SO3, NaCl, CO2
2) Which of the above compounds have
Molecular formula:
Ionic formula:
Distinct empirical formula:
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3) Indicating the type and number of atoms in a
molecule of the covalent compound: C6H12O6.
a. C:
b. H:
c. O:
d. Molecular formula:
e. Empirical formula:
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Simple Binary Molecular Compounds
H2O water (common name)
NH3ammonia (common name)
N2O dinitrogen oxide (nitrous oxide)
NO nitrogen monoxide (nitric oxide)
NO2 nitrogen dioxide
N2O4 dinitrogen tetroxide
CO carbon monoxide
CS2 carbon disulfide
SO3 sulfur trioxide
CCl4 carbon tetrachloride
PCl5 phosphorus pentachloride
SF6 sulfur hexafluoride
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4) Give systematic names to following binary inorganic
molecular compounds
a) H2O:
b) HCl:
c) SF6:
d) BF3:
e) N2O4:
f) CCl4:
g) SO3:
h) PCl3:
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5) Give the common name of the following molecular
compounds
a. NH3:
b.
CH3COOH:
c.
C6H12O6:
d.
C2H5OH:
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Naming Acids
Formula starts with acidic H
HCl Hydochloric acid
HNO3Nitric acid
H2SO4Sulfuric acid
HClO3Chloric acid
H3BO3Boric acid
H3PO4Phosphoric acid
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Names of acids and ions
HClO hypochlorous ClO ¯ ”hypochlorite”
HClO2 chlorous ClO2¯ “chlortie”
HClO3 chloric ClO3¯ chlorate
HClO4 perchloric ClO4¯ perchlorate
HNO3 nitric NO3 ¯ nitrate
HNO2 nitrous NO2 ¯ nitrite
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Naming bases
formula ends with OH
NaOH sodium hydroxide
Ba(OH)2 barium hydroxide
KOH potassium hydroxide
NH4OH ammonium hydroxide
Ca(OH)2 calcium hydroxide
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6) Give the names of the following acids
Formula
Name
Ion (s)
Formula
a) HNO3:
b) H3PO4:
c) HNO2:
d) H3PO3:
e) H2SO4:
f) H2CO3:
g) H2SO3:
h) CH3COOH:
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Name
Ions(s)
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Types of Chemical Formula
Molecular
Shows ratio of atoms each element in the
compound. E.g ethyl alcohol : C2H6O
Condensed
Shows groups of atoms bonded together in the
formula. E.g ethyl alcohol: CH3CH2OH
Structural
Shows bonding of important groups in the formu a
E.g ethyl alcohol:
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Hyd rocarbons and Alco hols
alkanes – C n H 2n+2 E.g. C 5 H 12 pentane
alkenes – C n H 2n E.g. C 2 H 4 ethene
alkynes – CnH2n-2 E.g. C2H2 ethyne
alcohols – ROH E.g C2H5OH ethanol
where R refers to the hydrocarbon radical backbone
created by substituting an -OH functional group for
a H atom in the hydrocarbon
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Models of Ethanol
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7) Given the structural formula of an organic compound,
write the for the following: CH3CHClCH2OH
a. molecular formula
b. condensed formula
c. structural formula
d. line formula
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Hydrocarbons
Catenation
The formation of chains of atoms of the same
e lement
. key feature of carbon permits a vast
This
number of compounds to exist.
Four types of hydrocarbons
1. Alkanes (saturated): single C-C bonds
2. Alkenes (unsaturated): double C=C bond
3. Alkynes (unsaturated): triple bond
4. Aromatic (unsaturated): benzene rings
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Alkanes CnH2n+2
methane – CH4
ethane – C2H6
propane – C3H8
butane – C4H10
pentane – C5H12
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hexane – C6H14
heptane – C7H16
octane – C8H18
nonane – C9H20
decane – C10H22
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Base names of hydrocarbons
Prefix Carbons
Meth- 1
Eth- 2
Prop- 3
But- 4
Pent- 5
Hex- 6
Hept- 7
Oct- 8
Non- 9
Dec- 10
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I see much
memorization in
your future!
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8) Name, molecular, condensed and line formula of straight
chain alkane (saturated hydrocarbons) or n-alkanes.
a. 4 carbon n-alkane:
b. 7 carbon n-alkane:
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What is an Isomer?
Compounds with the same number and type
of atoms but with different arrangements are
called constitutional isomers
Molecular Formula C5H12
Condensed formulas
CH3CH2CH2CH2CH3
CH3CH(CH3)CH2CH3
(CH3)4C
pentane
2-methylbutane
2,2-dimethylpropane
All are isomers of C5H12.
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Alkane Isomers is there a formula?
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9) Draw the structural formula of constitutional isomers of
butane with molecular formula C4H10.
a.
n-butane: CH3CH2CH2CH3
b.
isobutene: (CH3) 3CH
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Butane
Butane molecules are
present in the liquid
and gaseous states
in the lighter
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Classifying Organic Compounds
Examples
Hydrocarbons
Alcohols
Acids
Amines
Ketones
Aldehydes
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Functional Group
C and H only
R-OH
R-COOH
R-NH2
R(C=O)R’
R-CHO
Ending
-ane
-ol
-oic acid
-amine
-one
-al
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10) Classification and the name of the following
Classification
Name
a. CnH2n+2 where n is 8:
b. CH3CH2CH2CH2-OH:
c. CH3CH2CH2-COOH:
d. CH3CH2CH2CH2CH2CH2-NH2:
a. CH3CH2-(C=O)-CH3:
d) CH3CH2-CHO:
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11) Identify the classification or name of the
following biologically important molecules
a)
b)
c)
d)
e)
f)
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